A student wishes to determine the chloride ion concentration in a water sample at 25 °C using a galvanic cell constructed with a graphite electrode and a half-cell of AgCI(s) + e¯ → Ag(s) + Cl¯(aq) E°red = 0.2223 V And a copper electrode with 0.500 M Cu²* as the second half cell Cu2* (aq) + 2 e¯ → Cu(s) E°red= 0.337 V The measured cell potential when the water sample was placed into the silver side of the cell was 0.0903 V. What is the standard cell potential for this cell in V?

A student wishes to determine the chloride ion concentration in a water sample at 25 °C using a galvanic cell constructed with a graphite electrode and a half-cell of AgCI(s) + e¯ → Ag(s) + Cl¯(aq) E°red = 0.2223 V And a copper electrode with 0.500 M Cu²* as the second half cell Cu2* (aq) + 2 e¯ → Cu(s) E°red= 0.337 V The measured cell potential when the water sample was placed into the silver side of the cell was 0.0903 V. What is the standard cell potential for this cell in V?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. e Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. Do you have enough information to Yes calculate the cell voltage under standard No conditions? If you said it was possible to calculate the cell voltage, do so and enter your answer||V here. Round your answer to 3 significant digits.
Calculate the cell potential for the galvanic cell (in volts) in which the following reaction occurs at 25.0∘C, given than [Ti2+] = 2.773 M and [Au3+] = 0.582 M. Use Standard reduction potentials
Calculate the cell potential, at 298 K, for the following reaction under the conditions given.Pb(s) + Fe2+(aq, 0.0100 M) → Pb2+(aq, 0.150 M) + Fe(s) Pb2+(aq) + 2 e‒ → Pb(s) E°red = ‒0.13 VFe2+(aq) + 2 e‒ → Fe(s) E°red = ‒0.44 V Group of answer choices: ‒0.75 V ‒0.80 V ‒0.34 V ‒0.27 V ‒0.44 V ‒0.50 V
A student wishes to determine the chloride ion concentration in a water sample at 25 °C using a galvanic cell constructed with a graphite electrode and a half-cell of AgCl(s) + e → Ag(s) + Cl(aq) Eºred = 0.2223 V And a copper electrode with 0.500 M Cu²+ as the second half cell Cu²+ (aq) + 2 e → Cu(s) Eºred= 0.337 V The measured cell potential when the water sample was placed into the silver side of the cell was 0.0595 V. Write the balanced equation for the overall reaction in acidic solution.
Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. Mg(s) ∣ Mg2+(aq, 1.74 M) || Cu2+(aq, 0.0053 M) ∣ Cu(s)
Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.
What mass of material will be deposited at the cathode when a current of 10.5 A is applied for 2.0 hours to the following cell: Cr(s) | Cr² (aq) || Al*(aq) | Al(s)
Use the tabulated electrode potentials to calculate △Grxn for the following reaction at 25 °C2 Fe^3 (aq) + 3Sn(s) ---> 2Fe (s) + 3Sn^2 (aq)
Fe (s) +3 Au (aq) ^ + Fe log ^ 3+ +3 Au (s) For the first part, identify the oxidation half-reaction , identify the reduction half- reaction, identify the oxidizing agent, and identify the reducing agent under standard conditions. Next, calculate the standard cell potential, E for the reaction . cell E^ red +1.69 V Half-reaction Au^ + (aq) + e^ - Au (s) Fe^ 3+ (aq) + 3 e^ - Fe (s) -0.040 V Now , calculate the non- standard cell potential , when [Au^ + ]=0.0015 M and the [Fe^ 3+ ]= 0.033 M. After finding the cell potential , calculate the Gibb's free energy , AG Finally, calculate the equilibrium constant , K. Express your answers in two significant digits . Show your work for partial credit . Under non -standard conditions , is this reaction spontaneous or nonspontaneous ? Are reactants or products favored at equilibrium under non -standard conditions ?
Calculate the standard cell potential (E°cell) of a galvanic cell made of lead and cadmium. Then determine the non-standard cell potential (Ecell) if the molarity of the cadmium solution was 0.20 M, and the molarity of the lead solution was 0.10 M. The temperature of the cell is 300 K. Cd2+(aq) + 2e– → Cd(s) E° = –0.403 V Pb2+(aq) + 2e– → Pb(s) E° = –0.126 V E°cell = ______________ Ecell = ______________
A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 3 Cu²+ (aq) + 2Al(s) → 3Cu (s) +2A1³+ (aq) 2+ Suppose the cell is prepared with 4.04 M Cu²+ in one half-cell and 4.43 M A1³+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. x10 X 3 8 Ś
A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 3Cu2* (ag) +2A1 (s) –- 3Cu (s) + 2AI³* (aq) 2+ in one half-cell and 4.12 M Al" in the other. 3+ Suppose the cell is prepared with 3.11 M Cu Calculate the cell voltage under these conditions. Round your answer to 3 significant digits.